Answered: Sulfur dioxide is released in the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Sulfur dioxide is released in the combustion of coal. Scrub-bers use aqueous slurries of calcium hydroxide to remove the SO₂ from flue gases. Write a balanced equation for this reactionand calculate ΔS° at 298 K [ΔS° of CaSO₃(s) =101.4 J/molK]

Expert Solution

Step 1

Calcium hydroxide and sulfur dioxide reacts to form calcium sulfite and water. The reaction is an acid-base neutralization (or) neutralization reaction, where the base is $C a {(O H)}_{2}$ and the acid is SO₂. The balanced chemical reaction could be written as,

$S O_{2} (g) + C a {(O H)}_{2} (s) \overset{}{\to} C a S O_{3} (s) + H_{2} O (l)$

Step 2

The $∆ S °_{r x t n}$ of the reaction is calculated as,

$∆ {S °}_{r x t n} = (S °_{H_{2} O} + S °_{C a S O_{3}} - S °_{S O_{2}} - S °_{C a {(O H)}_{2}}) 1 m o l ∆ {S °}_{r x t n} = 69.94 J / K + 101.4 J / K - 248.1 J / K - 83.93 J / K ∆ {S °}_{r x t n} = - 160.15 J / K$

The $∆ S °_{r x t n}$ of the reaction is $- 160.15 J / K$ .

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